All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: A 2.50-L container is filled with 175 g argon.a. If the pressure is 10.0 atm, what is the temperature?

Solution: A 2.50-L container is filled with 175 g argon.a. If the pressure is 10.0 atm, what is the temperature?

Problem

A 2.50-L container is filled with 175 g argon.
a. If the pressure is 10.0 atm, what is the temperature?

Solution

We are asked to find the temperature at the given conditions. Since mass, volume and pressure are given, we will use the ideal gas equation to calculate for temperature.

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K

In the ideal gas equation, moles are needed but the mass of Argon (Ar) is given instead. We’ll calculate the moles of Ar using its mass and molar mass.

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